Net Ionic Equations and Reactions

This video tutorial explains how to write the balanced net ionic equation for the reaction between calcium chloride (CaCl2) and magnesium sulfate (MgSO4). It begins with balancing the molecular equation, followed by determining the solubility and states of the substances involved. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation. Finally, it identifies and removes spectator ions to derive the net ionic equation, ensuring charge and atom balance.

What is the first step in writing a balanced net ionic equation?

• Split compounds into ions

• Determine the solubility of compounds

• Balance the molecular equation

• Identify spectator ions

Which of the following is generally soluble in water?

• Magnesium sulfate

• Barium sulfate

• Calcium sulfate

• Lead sulfate

How should slightly soluble compounds be treated in net ionic equations?

• As if they are soluble

• As if they are insoluble

• As if they are liquids

• As if they are gases

What happens to calcium sulfate in a precipitation reaction?

• It remains in solution

• It dissolves completely

• It forms a gas

• It falls to the bottom of the test tube

What is the ionic charge of calcium in the net ionic equation?

• 2-

• 1-

• 2+

• 1+

Which ion is not split in the net ionic equation?

• Chloride ion

• Magnesium ion

• Calcium sulfate

• Sulfate ion

What is the purpose of removing spectator ions in a net ionic equation?

• To determine solubility

• To simplify the equation

• To balance the equation

• To identify the precipitate

Which ions are considered spectator ions in this reaction?

• Magnesium ions

• Sulfate ions

• Chloride ions

• Calcium ions

What is the net charge of the balanced net ionic equation?

• 2-

• 2+

• 1+

• 0

What is conserved in the balanced net ionic equation?

• Neither mass nor charge

• Both mass and charge

• Charge only

• Mass only